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D & F BLOCK ELEMENTS in 1 Shot: FULL CHAPTER COVERAGE (Concepts+PYQs) || Prachand NEET

YAKEEN・173 minutes read

The speaker highlights the importance of understanding transition elements, providing examples like iron and zinc. Emphasis is placed on electron configurations, oxidation states, and properties of transition elements for academic success.

Insights

Emphasizing active engagement and focus on the topic at hand is crucial for effective learning.
The significance of studying transition elements in the D&F block of chemistry is highlighted for comprehensive understanding.
Understanding the electron configurations of transition elements like zinc and iron is essential for academic success.
The importance of practical knowledge, memorization of properties, and electron configurations for D block elements is stressed.
Interstitial compounds formed by small atoms in metallic crystals exhibit increased hardness and conductivity, surpassing pure metals.
Knowledge of oxidation states, electrode potential values, and the reactivity of D block elements is essential for identifying oxidants and reducing agents.

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Recent questions

What is the focus of the lecture?
Transition elements in the D&F block.
Why are transition elements important?
For academic success and comprehensive understanding.
How many transition elements are there?
36 transition elements in the periodic table.
What are the exceptions among D block elements?
Zinc, cadmium, mercury, and copper-nickel.
Why is memorizing electron configurations crucial?
Essential for exams and academic success.

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Summary

00:00

"Mastering Transition Elements in Chemistry Lecture"

The speaker addresses the audience, emphasizing the importance of focusing on the topic at hand and avoiding distractions.
The speaker encourages the audience to engage with the content and participate actively.
The topic of discussion is the D&F block in chemistry, specifically focusing on transition elements.
The speaker highlights the significance of studying the NCERT textbook for a comprehensive understanding.
The lecture is expected to last for several hours, covering the D&F block thoroughly.
The removal of certain chapters in chemistry is mentioned, emphasizing the importance of the D block and P block.
The speaker stresses the need to understand the transition elements and their properties.
The definition of transition elements according to IUPAC is explained, focusing on the n-1d subshell.
Examples of transition elements like iron and zinc are provided to illustrate the concept.
The importance of complete knowledge and understanding of transition elements is emphasized for academic success.

15:46

"D Block Elements and Transition Metals"

Zinc's electron configuration is 4s^2 3d^10, with n-1 d complete in its ground state, making it stable in its oxidation state.
Zinc, cadmium, mercury, and copper-nickel are exceptions among D block elements, not considered transition elements.
There are 36 transition elements in the periodic table, excluding the four exceptions.
The total number of elements in the D block is 40, with 36 being transition elements.
Scandium is a transition element due to its incomplete n-1 d configuration, unlike zinc.
Overcoming backlogs in studies requires a dedicated timetable and prioritization.
Memorizing the electron configurations of D block elements is crucial for exams.
General electronic configurations for D block elements involve n-1 d and n s electrons.
Scandium's electron configuration is argon 4s^2 3d^1, with exceptions like chromium and copper.
Exceptional cases in electron configurations occur when electrons move to lower energy levels, as seen in chromium's configuration.

30:37

"F Block Elements: Electron Jumping and Exceptions"

Small energy gap exists due to easy electron jumping in f block elements
Exceptions seen in f block elements
Energy gap is less due to electron jumping
Addition of electron from 4D to 3D results in stable confinement
Notable individuals answering correctly: Eli, Himanshi, Vibha, Kafia, Khushi, Miss Maddie
Configuration sequence: 4s 3d 4, 4s 3d 5 (Manganese), 4s 2 3d 6, 4s 2 3d 7, 4s 2 3d 8, 4s 2 3d 9
Exception in configuration due to electron shifting from 4s to 3d
Exceptional cases in D series elements: Neo BM to Silver
Technetium's configuration discrepancy: 5s 1 4d 6 in 11th class NCERT, 5s 1 4d 5 in 12th class NCERT
Palladium's exceptional confinement: 5s 0 4d 10, important for exams and coordination compounds

44:01

Essential Chemistry Concepts for Understanding Properties

Remembering properties is essential for studying and understanding them thoroughly.
Electronically confined properties are experimental-based.
Practical knowledge is crucial, especially for chemistry.
Salt analysis is a significant chapter in practical chemistry.
The periodic table and chemical bonding are essential topics for revision.
D block elements have higher melting points compared to S block elements.
Metallic bond strength depends on the number of valence electrons participating in bonding.
Moving from scandium to chromium, the number of unpaired electrons increases, strengthening metallic bonding.
The number of unpaired electrons affects the melting point of elements in the D series.
Metallic bond strength and melting point decrease as the number of unpaired electrons decreases.

59:58

"Metallic Bonding and Oxidation States Explained"

4D ones are bigger than 3D ones, with 4D and 5D ones being similar in size.
The graphs of both types are stuck in a similar manner, with reasons like the half rule and Zarco rule.
The size similarity is due to the poor screening of F and A substellar electrons, leading to increased effectiveness and root effectiveness.
Effective memory and listening mind bell saver concepts are discussed, emphasizing the attraction power of the nucleus.
Metallic bonds are strong due to strong interatomic interactions from a large number of unpaired electrons in atoms.
Transition elements like zinc have low metallic bonding strength due to the absence of unpaired electrons.
Zinc, cadmium, and mercury are volatile metals with low melting and boiling points due to weak metallic bonding.
D block elements exhibit variable oxidation states, with elements like scandium and zinc showing specific oxidation states.
Scandium shows only the P3 oxidation state, while zinc shows only one oxidation state due to specific electron configurations.
The stability of oxidation states is determined by electrode potential values, with elements like chromium and manganese showing stable oxidation states based on their electron configurations.

01:15:41

Stable Oxidation States of Iron, Copper, Manganese

Iron is stable in +2 and +3 oxidation states only.
Iron compounds in some oxo groups are unstable.
Brown ring complex of iron is stable in +2 oxidation state.
Copper shows stable oxidation states in aqua medium.
Copper achieves pseudo inert gas confine in its stable oxidation states.
Copper +2 forms unstable compounds like CuI2.
Copper +2 is a good oxidizing agent.
Copper does not react with dilute acids to release hydrogen gas.
Manganese shows variable oxidation states.
Scandium remains stable in +3 oxidation state due to achieving argon confine.

01:31:29

"Stability and Oxidation States of Elements"

The text discusses the stability of zinc and its highest value in the context of electrode potential.
Zinc plate is stable due to its confinement in Zinc Plus2, which is pseudo inert gas.
Manganese plus2 achieves stability through half feed d5 confinement.
Iron's + 3 to P2 value is comparatively low due to its stability in the + P state.
D Block elements show higher oxidation states with oxygen over fluorine.
Oxygen is preferred over fluorine due to its tendency for multiple bond formation.
Mixed oxides like mn3 o4, fe3 o4, and co3 o4 are stable compounds.
The text mentions the amphoteric nature of certain compounds.
The order of Oxiderm Power is determined by the standard electrode potential.
Chemical reactivity and E Note Values increase with the Oxiderm Power.

01:48:42

Electrode Potential: Oxidants vs. Reducing Agents

Remember the standard electrode potential and distinguish between oxidants and reducing agents.
Titanium Plus2, Vedium Plus2, and Chromium PlusTwo are reducing agents.
Red TV mnemonic: Red for titanium, V for Vedium, and TV for titanium and Vedium, representing reducing agents.
Manganese Plus 3 and Cobalt Plus 3 are good oxidants.
Remember the values of electrode potential for identifying oxidants and reducing agents.
D block elements show variable oxidation states due to high ionic charge, small size, and availability of vacant orbitals.
Zinc does not show variable oxidation states easily, while Scandium sometimes follows complexation.
D block elements show catalytic properties due to their tendency to show variable oxidation states.
Iron + 3 acts as a catalyst in reactions involving iodide and sulfate ions.
Interstitial compounds are formed when small atoms like carbon, hydrogen, nitrogen, or boron get stuck in the empty spaces between metal atoms in metallic crystals.

02:07:03

"Interstitial Compounds: Hardness, Alloy Formation, Oxidation States"

The text discusses the formation of interstitial compounds when small atoms like hydrogen, carbon, nitrogen, and boron occupy interstitial sites in metal castles.
Interstitial compounds exhibit properties such as having higher melting points than pure metals, with the example of iron's melting point being surpassed by interstitial compounds.
The analogy of laying thick stones followed by fine stones on a road is used to explain the effective packing and increased hardness in interstitial compounds.
Interstitial compounds are noted for their hardness, exceeding that of pure metals, and retaining metallic conductivity while being chemically inert.
The text emphasizes the importance of alloy formation with metals of similar atomic sizes, exemplified by Alnico, an alloy of aluminum, nickel, and cobalt.
The discussion touches on German Silver as an example of an alloy and the significance of chemical inertness in metals like German Silver.
The text mentions the importance of maintaining a difference in metal atom sizes below 15% when creating alloys to ensure effective mixing and hardness.
The text highlights the formation of oxides by metals reacting with oxygen at high temperatures, with scandium being an exception in forming AO type oxides.
The highest oxidation state of metals in oxides is discussed, with examples like vanadium forming VO2 and titanium forming Ti2O7 in their highest oxidation states.
The text concludes with a focus on the relationship between the oxidation number of a metal and the increasing ionic character and chemical properties in bonding.

02:22:53

"Understanding Ionic Character and Oxides Chemistry"

Mn2O7 has ionic character, leading to a discussion on the order or names of these characters.
Fajan's Rule is mentioned, highlighting that as charges increase, polarization and polarizing power increase.
The text delves into the impact of increasing polarizing power, leading to a decrease in ionic character.
The discussion shifts to ionic bond fusions and the rule regarding increasing charges on harvesting.
The text explores the nature of oxides, emphasizing that positive oxidation states lead to increased electronegativity and acidic character.
The concept of amphoteric oxides is introduced, with examples like chromium oxide in different oxidation states.
The text elaborates on reactions involving chromic acid and chromate ions, emphasizing the acidic nature of compounds.
A detailed explanation is provided on the gradual change in properties from basic to amphoteric in vanadium oxides.
Practical instructions on the preparation of K2Cr2O7 are outlined, involving the fusion of chromite and sodium carbonate in the presence of air or oxygen.
The text concludes with a discussion on the color changes and solubility of K2Cr2O7, emphasizing the importance of understanding the chemical reactions involved.

02:38:19

Chemical properties of K2Cr2O7 and reactions

Bundles will be smaller if more than the comparison with X and three bundles will be equal.
Tetrahedral geometry is important and chromate is related to it.
K2Cr2O7 is a good oxidizing agent in acidic medium, turning orange.
The reaction with FeCl2 will convert K2Cr2O7 to Fe2, acting as a reducing agent.
Oxidation state changes from +6 to +3 in chromium, turning green.
Acidifying the medium with H2SO4 leads to green-colored compounds.
K2Cr2O7 is used in a drunk driver test, detecting alcohol presence.
SO2 reacts with K2Cr2O7, turning orange to green, indicating the presence of SO2.
Chromal chloride test differentiates chloride ions, turning paper reddish-brown.
KMnO4 and K2Cr2O7 release oxygen when heated, used in various reactions.

02:56:38

"KMnO4 Oxidation Reactions and Color Changes"

MnO2 is the focus, with any oxidant being suitable, including oxygen, ozone, KClO3, and KNO3.
The compound changes color from green to purple when added to an acidic medium, converting to KMnO4.
KMnO4, when heated, produces K2MnO4, MnO2, and O2.
KMnO4 acts as an oxidant, affecting the pH of the medium based on acidity or neutrality.
Reactions involving KMnO4 include its conversion to Mn2+ in acidic medium, appearing light pink in color.
KMnO4 oxidizes Fe2+ to Fe3+ and sulfide to SO2, with Mn2+ converting to Mn4+.
KMnO4 reacts with iodide to form Fe3+ or Fe2(SO4)3.
KMnO4 oxidizes thiosulfate to sulfate and Mn2+ to Mn4+, with Mn2+ converting to P4.
KMnO4 combined with Mn4+ results in a light pink color.
KMnO4 in neutral medium converts to Mn4+, appearing brown in color.

03:15:01

Electron Shifts in Confine Orbitals of Elements

Confine involves shifting electrons between 5d and 4f orbitals.
Elements with one electron in 5d include Cerium, Gedo, Niyama, and Lute Iam.
Gedo rule dictates the electron shift in 5d and 4f, affecting the confine.
Europium's confine shifts to 6s 5d 4f 7 due to one electron in 5d.
Thorium is an exception in confine, with 6d 1 5f 1 configuration.
Elements like Protactinium, Europium, and Neptunium have one electron in 6d.
Lanthanoids' confine involves shifting electrons between 6d and 5f.
General properties of Lanthanoids include decreasing size left to right.
Lanthanoids commonly show a +3 oxidation state.
Elements like Cerium, Thulium, and Turbium show a +4 oxidation state.

03:29:57

"Europium and Lanthanoids: Oxidation States and Properties"

Europium shows oxidation states of +2 and +3.
Europium can act as both an oxidizing and reducing agent.
Reduction in all +2 oxidation states acts as a reducing agent.
Cerium in oxidation states of +4 and +3 can act as an oxidant and analytical agent.
Lanthanoids are silvery white, soft, and turn rapidly in air.
Lanthanoids have typical metallic structures and are good conductors of heat and electricity.
Lanthanoids show colored solid-state and aqueous solution ions.
Lanthanoids in +3 and +4 oxidation states are diamagnetic due to f0 and f14 configurations.
Actinides are reactive, especially in powdered form, forming mixtures of oxides and hydroxides.
Stability of higher oxidation states increases down the group in the d block, with tungsten being the most stable.

03:47:52

Mastering NEET Block D: Focus on Coordination Chemistry

The theory needed to excel in NEET questions on block D can be found in the DPP, modules, and exercises provided. Practice is crucial, especially in coordination chemistry, as missing key lectures can result in missing out on potential questions. Coordination chemistry is expected to yield two to three questions, so it's essential to focus on it until the next lecture.

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